Use a table of Standard Reduction Potentials to predict if a reaction will occur

Question

Use a table of Standard Reduction Potentials to predict if a reaction will occur between Ag metal and I_2(s), when the two are brought in contact via standard half-cells in a voltaic cell. If a reaction will occur, write a balanced net ionic equation for the reaction, assuming that the product ions are in aqueous solution. If no reaction will occur, leave all boxes blank. Use a table of Standard Reduction Potentials to predict if a reaction will occur between Pb metal and Br_2(l), when the two are brought in contact via standard half-cells in a voltaic cell. If a reaction will occur, write a balanced net ionic equation for the reaction, assuming that the product ions are in aqueous solution. If no reaction will occur, leave all boxes blank. Use the table "Standard Reduction Potentials' located in the "Table's, to predict if a reaction will occur when Mn metal is put into a 1M aqueous Pb^2+ solution. If a reaction will occur, write a balanced net ionic equation for the reaction. If no reaction will occur, leave all boxes blank.

Explanation / Answer

(1) Between Ag and I2

E0Ag+/Ag = + 0.800 V

E0I2/I- = +0.536 V

Since Ag+ has more reduction potential, Ag can not reduce I2.

(2) Between Pb and Br2

E0Pb2+/Pb = - 0.126 V

E0Br2/Br- = + 1.087 V

Since Br2 has more reduction potential, it can oxidise Pb as follows,

Pb (s) + Br2 (l) ----------> Pb2+ (aq.) + 2 Br- (aq.)

(3) Between Mn and Pb2+ (1M)

E0Mn2+/Mn = - 1.18 V

E0Pb2+/Pb = - 0.126 V

Since Reduction potential of Mn2+ is lower than Pb2+, Mn replaces Pb2+ from its solution as follows.

Mn (s) + Pb2+ (aq.) -----------> Mn2+ (aq.) + Pb (s)

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